What is the number of faraday required to produce $0.18 \ g$ aluminium at cathode during electrolysis of molten $AlCl_3$ (in $F$)? (Molar mass of $Al = 27 \ g \ mol^{-1}$)

How many total Faraday currents will be required to obtain $1 \ mole$ of $Ag$,$Mg$,and $Al$ respectively?

On passing a current through $KCl$ solution,$19.5 \ g$ of potassium is deposited. If the same quantity of electricity is passed through a solution of aluminium chloride,the amount of aluminium deposited is ............ $g$

Faraday's laws of electrolysis are related to the

Calculate the amount of electricity required in coulombs to convert $0.08 \ mol$ of $MnO_4^{-}$ to $Mn^{2+}$. (in $C$)

Calculate the current (in $mA$) required to deposit $0.195 \ g$ of platinum metal in $5.0 \ hours$ from a solution of $[PtCl_6]^{2-}$ : (atomic weight : $Pt = 195$)